Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • School
  • Show that for a first order reaction, time required for completion of 99% of reaction is twice the time required for complrtion of 90% of reaction.       <div style="

Show that for a first order reaction, time required for completion of 99% of reaction is twice the time required for complrtion of 90% of reaction.

 

 

 

 
 
 
 
 

Answers (1)

Time = \frac{2.303}{K}log \frac{initial concentration}{final concentration}

for 99% completion of reaction:

T_{1}= \frac{2.303}{K}\times \log \frac{100}{100-99}=\frac{2.303}{K}\times \log \frac{100}{1}= \frac{2 \times 2.303}{K}

for 90% completion of reaction:

T_{2}= \frac{2.303}{K}\times \log \frac{100}{100-90}=\frac{2.303}{K}\times \log 10= \frac{1 \times 2.303}{K}

\therefore T_{1} = 2\times T_{2}

Posted by

Sumit Saini

View full answer

Crack CUET with india's "Best Teachers"

  • HD Video Lectures
  • Unlimited Mock Tests
  • Faculty Support
cuet_ads

Similar Questions

Trending Articles/News

anam-khan

Supreme Court to hear plea against CBSE evaluation policy for Gulf Class 12 students on July 14
anam-khan

'Award grace marks': CBSE's July 28 supplementary exam sparks student outrage over college admissions
anam-khan

CBSE Class 12 supplementary exam 2026 on July 28; LOC submission starts

Latest Question